Chapter 1 basics 1. For an isotope of argon (Z = 18), the mass number is Chapter 2 Nuclearchemistry 40.

The number of neutrons in this isotope is: 1. The relative penetrating powers of a- and b18 40 22 the same as in any other isotope of argon particles, g radiation and neutrons (n) are: a > b > g > n n> g > b > a n> a > b > g 2. Allotropes of sulfur include: 32S and 34S S8 and S6 n< a < b < g S and [S ]2+ S in different oxidation states
8 8

3. Energy is inversely proportional to: wavelength frequency wavenumber Planck's constant 4. How many radial nodes does a 3p atomic orbital possess? 0 1 2 3 5. Which of the following atomic orbitals can overlap with an atomic orbital of the same type on an adjacent atom (both atoms lie on the x axis ) to give a π bond? 2px 3dxy 2s 3px 6. Which of the following atomic orbitals contains one nodal plane? 3s 3py 3dz2 3dxy 7. An atom with a valence electronic configuration of 1s22s22p63s23p3 belongs to group 3 5 11 15 8.An element has an outer ground state electronic configuration of 4s13d10. The element: is a metal is a non-metal is in group 10 is a liquid at 298 K 9. Sketch an MO diagram to describe the bonding in [He2]2+. From the result, you can say that: the ion is paramagnetic the ion has a bond order of zero the ion is likely to be less stable than He2 the ion is diamagnetic

2. An a - particle is: He2+

[He2]2+
234

He+ U92 is

He

3. The product of the a-decay of 230 U92 234Np93 230Th90 234Th90

4.The half-life of 222Rn is 3.82 days. The decay constant, k, is: 1.26 x 10–4 s–1 5.47 x 10–5 s–1 –7 –1 –6 –1 9.12 x 10 s 2.10 x 10 s 5.The decay of a radioactive isotope (assuming that there is no complication by decay of a daughter nuclide) follows: first order kinetics zero order kinetics second order kinetics no particular type of kinetics 6.Which of the following are transuranium elements? Pa, Np, Am Ac, Am, Bk Cf, Bk, No Th, Pu, Cm 7. Which of the following elements is not man-made? Es Bh U No

8. Deuteration of C2H5OH to C2H5OD: shifts the wavenumber for the O–H/D stretch to a higher value shifts the wavenumber for the O–H/D stretch to a lower value has no effect on the absorption due to n(O–H/D) dramatically alters all absorptions in the IR spectrum of the compound 10. The correct ordering of the electronegativities of the following atoms is: 9. The nuclear spins of 1H and 2H are, respectively: ½ N<O<H H<N<O H<O<N O < N < H and 1 ½ and ½ 1 and ½ ½ and 0 11. Atoms of the elements N and P have: the same 10. The 19F NMR spectroscopic signal of NH4PF6 is a: number of valence electrons the same number of doublet septet sextet singlet protons the same number of electrons the same number of neutrons 11. The 11B{1H} NMR spectrum of H3B.PF3 is a: doublet singlet doublet of quartets doublet of 12. How many radial nodes does a 5f orbital possess? quartets of quartets 1 0 3 5 12. You are trying to distinguish between Ph2PH 13. For which of the following molecules would (compound A) and Ph2PCH2PPh2(compound B) VSEPR theory predict a trigonal pyramidal structure? using 31P NMR spectroscopy. You would: see one PF3 BF3 ClF3 BrF3 signal for A and two for B. be able to readily 14. Which of the following molecules is non-polar? 31 31 distinguish A by running P and P{1H} NMR spectra. BCl3 SO2 H2S OF2 see a doublet in the 31P NMR spectrum of A but a triplet for B, both with large values of JPH. not be able 15. Sketch an MO diagram for O2. Using the to distinguish the compounds by this method. information in the diagram, which statement is incorrect? 13. 195Pt is spin-active with I = ½ (33.8%). The 31P{1H} O2 is diamagnetic The bond order in O2 is 2 NMR spectrum of cis-[PtCl2(PPh3)2] would exhibit: The bonding in O2 has a π-component. The bonding in O2 has a σ-component

a doublet superimposed on a singlet a binomial triplet a doublet two doublets 14. If you were to record the solution 31P{1H} NMR spectrum of the octahedral complexmer-[IrCl3(PEt3)3], the spectrum (assuming isotopes of Ir are not spin active) would exhibit: a doublet and a triplet with relative integrals 2:1 a doublet and a triplet with relative integrals 1:2 a singlet two singlets with relative integrals 2:1 15. WCl2F4 has an octahedral structure. Which of the following statements about the 19F NMR spectra of cisand trans-WCl2F4 is not true. Ignore coupling to 183W. The spectrum of trans-WCl2F4 contains two signals 16. The spectrum of trans-WCl2F4 contains one signal The spectrum of cis-WCl2F4contains two triplets, relative integrals 1:1 A value of J(19F-19F) can be measured from the spectrum of cis-WCl2F4 Chapter 4: Bonding in polyatomic molecules 1. Appropriate hybridization schemes for the C atoms in molecular CH3CO2H are sp3 and sp 3 2 2 sp and sp sp and sp sp3 and sp3 2. sp3 hybridization would not be appropriate for the central atom in: SiF4 [PCl4]+ XeF4 [Me4N]+ 3.In the equation for the normalized wavefunction: y sp = Ny2s + Ny2p, N =? ½ 1
1

bonds. B-H terminal bonds cannot be considered as 2c-2e interactions. The observed structural parameters in B2H6 suggest the presence of a localized B-B interaction. 12. An MO diagram for a model compound XH6 (Oh) can be constructed by considering the interactions between the orbitals of atom X and the LGOs for the Oh H6 fragment. What are the correct symmetry labels for these LGOs? a1g, t1u, eg a1g, t2g, eg a1, t1, e a1, t2, e 13. The bonding in XH3 can be considered in terms of the interactions between the orbitals of atom X and the LGOs of the H3 fragment. For the LGOs, when X = B, the in-phase combination of H 1s orbitals has a1' symmetry, but when X = N, it has a1symmetry. This is because: NH3 has C3v symmetry, but BH3 belongs to the D3h point group. NH3 has D3h symmetry, but BH3 belongs to the C3v point group. NH3 has C3v symmetry, but BH3 belongs to the D3d point group. NH3 has C3 symmetry, but BH3 belongs to the C3v point group. 14. The bonding in [NO3]– can be considered in terms of a set of three resonance structures which describe the predominant contributions to the bonding. Which statement is incorrect about this set of resonance structures? Each resonance structure possesses two localized N=O double bonds. N carries a formal positive charge in each resonance structure. The set of resonance structures has to account for the equivalence of the N–O bonds. The N atom obeys the octet rule in each resonance structure.

/√2 √2

4. sp hybridization for the C atom in CS2 is all that is required to allow for : the formation of two C=S bonds the formation of the s components of two double bonds the formation of two s bonds and two p bonds the formation of a s bond and accommodation of one lone pair

7. Look at Figure 4.19 in Inorganic Chemistry. Which property does each of the eorbitals not possess? Lone pair character. N–H bonding character. One nodal plane. No contribution from one H 5. In an MO diagram for the formation of H2O in which the z axis bisects the H–O–H angle: the O 2pz atomic 1s orbital orbital interacts with an in-phase combination of H 8. Look at Figure 4.21 in Inorganic Chemistry. Which 1s atomic orbitals the O 2pz atomic orbital statement is not true? All the bonding MOs involve C interacts with an out-of-phase combination of H and H character. There are 4 bonding and 4 1s atomic orbitals the O 2pz atomic orbital is non- antibonding MOs. The molecule of diamagnetic. bonding the O 2s atomic orbital is non-bonding All the bonding MOs are equivalent 6. In monomeric BH3, let an axis definition place the 9. Look at Figures 4.27 and 4.28 in Inorganic molecule in the xz plane. Which atomic orbital on B is Chemistry. Which statement is not true? non-bonding? 2s 2px 2py 2pz All six S–F bonds in SF6 are equivalent. A reasonable bonding picture for SF6 can be developed 10. Which statement is true about the bonding in B2H6? using an S basis set of 3s and 3p orbitals. The A localized bonding picture can be developed for S–F bond order is 1. SF6 is diamagnetic B2H6 in which each B atom obeys the octet rule. Bonding pictures for B2H6 involve multicentre bridge

Chemistry, the value of ΔlatticeHo(NaCl,s) (defined for Chapter 5: Structures and energetics of metallic and the formation of NaCl) is determined to be: –1485 kJ mol–1 –787 kJ mol–1 +1485 kJ mol–1 ionic solids –1 +787 kJ mol 1. Which statement is incorrect about a cubic closepacked lattice? All atoms have a coordination number 9. Which of the following statements is incorrect of 12. Layers of close-packed atoms are stacked in Madelung constants for MX2 lattices are greater than those for MX lattices. Use of the Born-Landé an ABCABC... pattern. Layers of close-packed equation is restricted to lattices for which an atoms are stacked in an ABABAB... pattern. electrostatic model is appropriate. Madelung The packing is more efficient than in a body-centred constants are structure dependent. A lattice cubic lattice energy is an internal energy change, and latticeU(0 K) 2. The coordination numbers of spheres in body-centred = latticeH(298 K). cubic, simple cubic and cubic close-packed lattices are, – respectively: 8, 6, 12 6, 8, 12 6, 12, 8 8, 12, 12 10. Ions such as [CN] may be regarded as being spherical in some lattices. This is because: each ion 3. Look at Table 5.2 in Inorganic Chemistry. Use the is approximately spherical the ions are freely data to estimate the metallic radius of Ba in metallic rotating the ions are in random orientations barium at 298 K. The value (in pm) is: the ions are either freely rotating or in random 231 217 215 197 orientations 4. Which statement is true? The electrical conductivity 11. The coordination nos of Ti(IV) and O2– in rutile are, of a metal increases with temperature. The respectively: 6 and 3 3 and 6 2 and 4 4 and 2 electrical conductivity of a semiconductor increases with temperature. The resistivity of a semiconductor 12. An example of a compound that crystallizes with a layer structure is: CdI2 CaF2 ZnS SnO2 increases with temperature Metals and semiconductors have similar electrical conducting 13. Na2S crystallizes with an antifluorite structure. properties Which statement is true about this structure? The coordination number of each S2– centre is 8. 5. The behaviour of metals and semiconductors is Each Na+ ion is within a cubic arrangement of S2– ions. usually discussed in terms of band theory. Which statement is not true? A partially filled band is The structure is based on an CaF2 structure, with2+ Na+ ions in Na2S occupying the same sites as Ca ions characteristic of a metal. Doping Si with As in CaF2. The S2– ion is tetrahedrally sited. enhances its semiconducting properties. Band gaps vary among different semiconductors but are always relatively large. Band gaps for insulators are large 6. Which statement gives incorrect information about the formation of NaCl(s) from Na(s) and Cl2(g)? Na is oxidized and Cl reduced. An ionic lattice forms. Both the ionization of Na and electron attachment to Cl are exothermic processes. When NaCl forms from its gaseous ions, energy is released. 7. Which statement is true about an XY2 lattice: the coordination number of X2n+ is twice that of Yn– the coordination number of X2n+ is half that of Yn– the unit cell contains twice as many X2n+ ions as Yn– the coordination environments of X2n+ and Yn– are the same. 8. The standard enthalpy of formation of NaCl is –411 kJ mol–1. Using data from the appendices of Inorganic 14. Which statement is incorrect? CaO crystallizes with the CsCl structure. Wurtzite and zinc blende are polymorphs of ZnS. β-Cristobalite is one crystalline form of SiO2. CaTiO3 (perovskite) is an example of a double oxide 15. A unit cell of ReO3 consists of a cubic arrangement of Re atoms with O atoms centred along each edge of the cube. The coordination number of each Re atom is: 6 3 8 2 Chapter 6 Acids bases ions and aqueous solutions 1. In group 1, values of the first ionization energies follow the order Li > Na > K Na > K ≈ Rb ≈ Cs K > Na > Li Rb > K > Na 2. In group 1, values of the metallic radii follow the order: Li > Na > K Na < K < Rb K > Rb > Cs Cs < K < Li

14. The enthalpy change for the dissociation: M2(g) → 2M(g) is: more positive for Li2 than for K2 more positive for Rb2 than for K2 more positive for Na2 than for Li2 more positive for Cs2 than for K2 15.Which statement is true? Cs reacts explosively with H2O Li reacts explosively with H2O Rb does not react with H2O The reaction between K and H2O is less vigorous than that of Na and H2O 16. Which two chemicals are manufactured on a large scale in the chloralkali industry? Na and Cl2 NaCl and Cl2 NaOH and Cl2 NaCl and NaOH 17. The Downs process is used: to manufacture NaOH to electrolyse molten NaCl as the main manufacturing process for Cl2 to manufacture NaCl 18. Which one of the following salts is sparingly soluble in water, the other salts being readily soluble? LiCl LiNO3 Li2CO3 LiI

8. When alkali metal ions are complexed with the cyclic 19. Na2O reacts with water to give: NaOH as the only ether 18-crown-6, the most stable complex is formed product NaOH and H2O2 NaOH and O2 with: Li+ Na+ K+ Rb+ NaOH and H2 9.The equilibrium: 2Na = Na+ + Na– can be shifted to the right-hand side by: carrying out the reaction in liquid NH3 adding THF (a monodentate cyclic ether) to complex the cation adding 18-crown-6 (a hexadentate cyclic ether) to complex the cation forming a cryptate complex 10. Sodium amalgam is used as: an oxidizing agent a reducing agent a drying agent a source of Na– 20. Which is exothermic? K(g) + e- → K-(g) K(g) → K+(g) + e→ K(g) K+(aq) → K+(g) Chapter 7: Reduction and oxidation 1. In which of the following is the metal reduced? (These are not balanced equations). [Fe(CN)6]4– [Fe(CN)6]3– [MnO4]– MnO2 2– – 2– [MnO4] [MnO4] [Cr2O7] [CrO4]2– K(s)

11. Of the options given below, which is the safest way to dispose of Na metal? Add small amounts of Na to + 2+ propan-2-ol Add small amounts of Na to ethanol 2.o For the cell: 2Ag (aq) + Zn(s)o 2Ag(s) + Zn (aq) E cell = 1.56 V. The value of ΔG is: Add small amounts of Na to propan-1-ol Add 150 kJ per mole of Zn –602 kJ per mole of Ag small amounts of Na to water –301 kJ per mole of Ag –301 kJ per mole of Zn 12. Na3N adopts an anti-ReO3 structure. Which o (350 K) = –72 kJ mol–1, the value of K is statement is true about the unit cell of Na3N? N3– ions 3. If ΔG10 5.6 x 10 4.2 x 1012 5.5 x 1024 1.2 x 1029 occupy corner sites Na+ ions occupy corner sites N3– ions occupy edge sites Na+ ions occupy face 4. For a thermodynamically spontaneous cell reaction, sites which statement is correct? Eo (reduction) o Eo 13. HPMA (hexamethylphosphoramide,) is used in the must be more negative than E (oxidation). o synthesis of lithium-containing compounds under non- (oxidation) must be more negative than E (reduction). o E cell should be negative. The difference between Eo aqueous conditions. Which statement about HMPA is (reduction) and Eo (oxidation) must be more than 1.0 V incorrect? HMPA is a non-coordinating solvent HMPA is polar HMPA dissolves LiBr 5. Use Appendix 11 in Inorganic Chemistry to HMPA has the potential to form hydrogen bonds determine Eocell for the reaction: Cl2 + 2Br– 2Cl– + Br2 The value is: –2.45 V –0.27 V 0.27 V 2.45 V

integrals 2:1 15. The spectrum of trans-WCl2F4 contains two signals Answers 1. ClF3 2. a C2 axis 3. SO3 4. H2S and OF2 5 NH3 6 XeF4 . 7. C2v 8 C2v 9 XeF4 10 [PF6]– 7.pH affects the E value for: the reduction of [Cr2O7]2– 11SF5Cl 12. The point group changes from D3h to Td to Cr3+ the reduction of Cr3+ to Cr2+ the reduction of 13. 4 vibrational modes, 2 of which are degenerate 14. 9. 15. Symmetric stretch; asymmetric stretch (doubly Cr2+ to Cr the reduction of Cr3+ to Cr degenerate); one absorption 8. Look at Figure 7.2 in Inorganic Chemistry. In Chapter1 answers? alkaline solution, the value of Eo (at pH 14) for the Covalent NaCp is formed. is polymeric with reduction of [MnO4]– to Mn(OH) 2 is: tetrahedral Be. Tetrahedral It is sparingly soluble +0.63 V +0.55 V +0.34 V +1.69 V in water In Al2Ph4(µ -C≡ CPh)2, the bridge bonds can be 9.Look at Figure 7.4 in Inorganic Chemistry. Carbon will reduce FeO to Fe at: 1500 K 900 K 700 K 500 K described in a similar way to those in Al2Me4(µ -Ph)2. Ph > Me polymeric with trigonal bipyramidal Pb. R3As from AsCl3 and a suitable Grignard reagent; R5As from oxidative addition of Cl2 to R3As and treatment 11. Look at the representations of the MOs in Figure with RLi. {(Me3Si)2CH}4Sn2; the Sn2C4 unit is non4.23 in Inorganic Chemistry. Which statement about planar. Me2GeCl2 + 2Li Me2Ge + 2LiCl these MOs is incorrect? The a2'' MO does not possess In the solid state, Cp2Pb has a polymeric structure B–F bonding character. The e' MO contains a [(C5Me5)2Ga]+ is isostructural with [(C5Me5)2Al]+. nodal plane. The a1' MO has B–F σ-bonding The product contains the [Ph3C]+ ion. character. The e' MO is one of a pair of degenerate Cp2Mg is monomeric. MOs. A diamagnetic salt is formed 15.Figure 4.29 in Inorganic Chemistry gives an MO Chapter 3 Symmetry diagram for the formation of [HF2]–. Which statement 1. Which of the following does not contain a C3 axis? is incorrect about this bonding picture? The bond order POCl3 [NH4]+ [H3O]+ ClF3 of each H–F bond is 1. There is one MO with 2.Which symmetry elements does cis-N2F2 contain? net bonding character. The bonding can be a C2 axis a h plane an inversion centre, I an S2 axis described as a 3-centre 2-electron interaction. 3. Which if the following species possesses The σg* MO contains 3 nodal planes. both C3 and C2 axes? SO3 NH3 PCl3 [H3O]+ Answers chapter 4 3 2 1 4. Which two species belong to the same point group? 1. sp and sp 2. XeF4 3. /√2 4. the formation of the σ components of two double bonds XeF2 and OF2 H2O and CO2 H2S and OF2 5. the O 2pz atomic orbital interacts with an in-phase [NO2]+ and [NO2]– 6. Use Appendix 11 in Inorganic Chemistry for this question. For a Cu2+(aq) / Cu(s) half-cell (at 298 K) in which [Cu2+] = 0.02 mol dm–3, E is +0.44 V +0.39 V +0.29 V +0.24 V
combination of H 1s atomic orbitals 6. 2py 7. lonepair character 8. All the bonding MOs are equivalent. 9. The S–F bond order is 1. 10. Bonding pictures for B2H6 involve multicentre bridge bonds. 11. The a2'' MO does not possess B–F bonding character. 12. a1g, t1u, eg 13. NH3 has C3v symmetry, but BH3 belongs to the D3h point group 14. Each resonance structure possesses two localized N=O double bonds 15. The bond order of each H–F bond is 1.

5. Which of the following belongs to the C3v point group? SO3 BBr3 NH3 AlCl3 6. Which molecule does not have Td symmetry? SiF4 P4 CH4 XeF4 7.Which molecule or ion has D3h symmetry? [H3O]+ CHCl3 [CO3]2– NF3 8. SO2 belongs to which point group? C2v C2 D∞h C2h 9. Which of the following molecules or ions possesses a C4 principal axis? XeF4 CF4 SF4 [PF4]+ 10. Which of the following molecules or ions possesses an inversion centre (centre of symmetry)? [PF6]– SiH4 BF3 PF5

11. Which of the molecules or ions belongs to the C4v point group? SF5Cl [BH4]– XeF4 trans-WCl2F4 12. Which statement is true about the change in symmetry on going from BF3 to [BF4]–? The point group changes from D3h to Td The point group changes from C3v to Td The point group changes from D3h to D4h The point group changes from D3h to C3v 13. CO2 has: 3 vibrational modes modes, 2 of which are degenerate only an IR active symmetric stretch 4 vibrational stretching modes

14. The number of degrees of vibrational freedom possessed by CH4 is: 10 6 4 9 15. Which of the following gives the correct description of the vibrational modes of SO3, and how many absorptions do these vibrational modes give rise to in the IR spectrum of SO3? Symmetric stretch; asymmetric stretch (doubly degenerate); one absorption Symmetric stretch; asymmetric stretch (doubly degenerate); two absorptions Symmetric stretch; asymmetric stretch; two absorptions Symmetric stretch; asymmetric stretch; one absorption